The half‑equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.440 moles of a monoprotic weak acid ( K a = 8.3 × 10 − 5 ) is titrated with NaOH , what is the pH of the solution at the half‑equivalence point?

Answer : The pH of solution at the half‑equivalence point is, 4.1

Explanation :

As we known that the titration takes place between strong base and weak acid.

So, at half‑equivalence point of a titration the pH of the solution is equal to the of weak acid.

As we are given:

Now we have to calculate the value of .

The expression used for the calculation of is,

Now put the value of in this expression, we get:

Thus,

Therefore, the pH of solution at the half‑equivalence point is, 4.1

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answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.